If 2.00g of p-aminophenol (109.1 g/mol) reacts with 5.00 ml of acetic anhydride (102.1 g/mol and density = 1.08 g/ml), what mass of acetaminophen (180.2 g/mol) would be made? show all calculations.

The complete reaction is as,

4-Aminophenol + Acetic Anhydride → Acetaminophen + Acetic Acid

First of all convert the ml of Acetic anhydrite to grams,

As,

Density = mass / volume

Solving for mass,

mass = Density * Volume

Putting values,

mass = 1.08 g/ml * 5ml

mass = 5.4 g of acetic anhydride

First Find amount of acetic anhydride required to react completely with 2 g of p-Aminophenol,

As,

109.1 g of p-aminophenol required = 102.1 g of acetic anhydride

so, 2 g of p-aminophenol will require = X g of Acetic Anhydride

Solving for X,

X = (2 g * 102.1 g) : 109.1 g

X = 1.87 g of acetic anhydride is required to be reacted.

But, we are provided with 5.4 g of Acetic Anhydride, means p-aminophenol is the limiting reactant and it controls the formation of product. Now Let's calculate for product,

As,

109.1 g of p-aminophenol produced = 180.2 g of Acetaminophen

So 2.00 g of p-aminophenol will produce = X g of Acetaminophen

Solving for X,

X = (2.00 g * 180.2 g) : 109.1 g

X = 3.30 g of Acetaminophen

Result:

If 2.00g of p-aminophenol reacts with 5.00 ml of acetic anhydride 3.30 g of acetaminophen is made.